Sigma Bonding Ao bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH4 1s orbital What atomic or hybrid orbital on O makes up the sigma bond between O and H in water, H,O? orbital on O What is the approximate H-O-H bond angle? Submit Answer Try Another Version 10 item attempts remaining

Sigma Bonding Ao bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH4 1s orbital What atomic or hybrid orbital on O makes up the sigma bond between O and H in water, H,O? orbital on O What is the approximate H-O-H bond angle? Submit Answer Try Another Version 10 item attempts remaining

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter3: Electron Orbitals

Section: Chapter Questions

Problem 8E

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Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central nitrogen atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order does the MO model predict for the NO bonds in the nitrite ion?
Sketch the molecular orbital and label its type ( or , bonding or antibonding) that would be formed when the following atomic orbitals overlap. Explain your labels. a. b. c. d.
Which of the p orbitals do you think contributes the most inthe mixing that leads to the right-most sp3 hybrid orbital in thesecond row of the figure?
The following is part of a molecular orbital energy-level diagramfor MOs constructed from 1s atomic orbitals. (a) What labels do we use for the two MOs shown? (b) Forwhich of the following molecules or ions could this be theenergy-level diagram:H2, He2, H2+, He2+, or H2-?(c) What is the bond order of the molecule or ion? (d) If anelectron is added to the system, into which of the MOs will itbe added? [
Represent the bonding in each molecule or ion by drawing the orbitals (hybridized and unhybridized) of each atom in the bond. Label the σ and π bonds and label each bond by the orbitals that it is made from. For instance, the C–H bond in CH4 would be made from the overlap of: C (sp3) – H (1 s). You may draw the hybridized sigma orbitals as sticks and the unhybridized p-orbitals as lobes for clairity and ease. a. HONO b. CH3 CCH c. C3 H4 d. C2 O4 2-
Draw a picture that shows all three 2p orbitals on one atomand all three 2p orbitals on another atom. (a) Imagine theatoms coming close together to bond. How many s bondscan the two sets of 2p orbitals make with each other? (b) Howmany p bonds can the two sets of 2p orbitals make with eachother? (c) How many antibonding orbitals, and of what type,can be made from the two sets of 2p orbitals?
Draw a picture that shows all three 2p orbitals on one atomand all three 2p orbitals on another atom. (a) Imagine theatoms coming close together to bond. How many σ bondscan the two sets of 2p orbitals make with each other? (b) Howmany π bonds can the two sets of 2p orbitals make with eachother? (c) How many antibonding orbitals, and of what type,can be made from the two sets of 2p orbitals?
1. Why is the concept of hybridization necessary in the first place?a. because the bonding of some atoms using their unhybridized orbitals will not lead to the expected geometryb. Because of the electrons of an atom are shielding the outermost electron from the nucleus, thereby, reducing the effective nuclear chargec. Because of the octet ruled. Because of the orbitals of an atom need to respond accordingly to give the highest energy possible2. which of the following would the bonding be WEAKENED with adding an electron from the negative molecular ion?a. N2b. C2c. B2d. All of these
Construct an approximate molecular orbital energy diagram for a hypothetical planar form of NH3. From a consideration of the atomic energy levels, place the N and H3 orbitals on either side of a molecular orbital energy-level diagram. Then use your judgement about the effect of bonding and anti bonding interactions and energies of the parent orbitals to construct the molecular orbital energy levels in the centre of your diagram and draw lines indicating the contributions of the atomic orbitals to each molecular orbital. Ionization energies are I(H1s) = 13.6 eV, I(N2s) = 26.0 eV, and I(N2p)=13.4 eV.
Consider the H2+ ion. (a) Sketch the molecular orbitals ofthe ion and draw its energy-level diagram. (b) How manyelectrons are there in the H2+ ion? (c) Write the electronconfiguration of the ion in terms of its MOs. (d) What isthe bond order in H2+? (e) Suppose that the ion is excitedby light so that an electron moves from a lower-energy toa higher-energy MO. Would you expect the excited-stateH2+ ion to be stable or to fall apart? (f) Which of the followingstatements about part (e) is correct: (i) The light excitesan electron from a bonding orbital to an antibonding orbital,(ii) The light excites an electron from an antibonding orbitalto a bonding orbital, or (iii) In the excited state there are morebonding electrons than antibonding electrons?
The O¬H bond lengths in the water molecule 1H2O2 are0.96 Å, and the H¬O¬H angle is 104.5°. The dipole momentof the water molecule is 1.85 D. (a) In what directionsdo the bond dipoles of the O¬H bonds point? In what directiondoes the dipole moment vector of the water moleculepoint? (b) Calculate the magnitude of the bond dipoleof the O¬H bonds. (Note: You will need to use vector addition to do this.) (c) Compare your answer from part (b)to the dipole moments of the hydrogen halides (Table 8.3).Is your answer in accord with the relative electronegativityof oxygen?
The lactic acid molecule, CH3CH1OH2COOH, gives sourmilk its unpleasant, sour taste. (a) Draw the Lewis structurefor the molecule, assuming that carbon always forms fourbonds in its stable compounds. (b) How many p and howmany s bonds are in the molecule? (c) Which CO bond isshortest in the molecule? (d) What is the hybridization ofatomic orbitals around the carbon atom associated withthat short bond? (e) What are the approximate bond anglesaround each carbon atom in the molecule?